Which of the following elements will have the highest electronegativity?

  • Chlorine 

  • Nitrogen 

  • Cesium 

  • Fluorine

How does electron affinity change when we move from left to right in a period in the
periodic table?

  • Generally increases

  • Generally decreases

  • Remains unchanged

  • First increases and then decreases

One mole of magnesium in the vapour state absorbed 1200 kJ mol-1 of energy.

If the first and second ionization energies of Mg are 750 and 1450 kJ mol-1 respectively,

the final composition of the mixture is

  • 86% Mg+ + 14% Mg2+ 

  • 36% Mg+ + 64% Mg2+ 

  • 69% Mg+ + 31% Mg2+ 

  • 31% Mg+ + 69% Mg2+ 

The atomic species that has the maximum ionization energy is : 
  • O-
  • S-
  • Se-
  • Te-

Ionic radii are :

  • Inversely proportional to effective nuclear charge.

  • Inversely proportional to square of effective nuclear charge.

  • Directly proportional to effective nuclear charge.

  • Directly proportional to square of effective nuclear charge.

An atom has electronic configuration is 1s2 2s2 2p6 3s2 3p6 3d3 4s2 , you will place it in :

  • V group

  • XV group

  • II group

  • III group

Which of the following oxide is amphoteric in nature?

  • SnO

  •  SiO2

  •  GeO2

  •  CO2

The increasing order of non-metallic character of the elements N, P, O, and S is: 

  •  P < S < N < O

  • O < S < N < P 

  • O < N < S < P 

  • N < S < O < P

The correct order of metallic character of elements B, Al, Mg and K  is :

  • B > Al > Mg > K

  • Al > Mg > B > K

  • Mg > Al > K > B

  • K > Mg > Al > B

Considering the elements B, C, N, F, and Si; the correct order of their non-metallic character is :

  • B > C > Si > N > F

  • Si > C > B > N > F

  • F > N > C > B > Si

  • F > N > C > Si > B

The correct order of their chemical reactivity of the elements F, Cl, O and N in terms of oxidizing property is :

  • F > Cl > O > N

  • F > O > Cl > N

  • Cl > F > O > N

  • O > F > N > Cl

Incorrect statement among the following is-

  • Elements are classified into periods and groups

  • Elements with similar properties are placed in the same group

  • This makes the study of elements simpler

  • Elements are placed according to decreasing atomic number

The maximum number of elements that can be accommodated in the sixth period are :

  •   8

  • 18

  • 32

  • 4 16

The element named after Lawrence Berkeley Laboratory is 

  • Seaborgium

  • Lawrencium

  • Moscovium

  • Hafnium

 B has lesser ionization enthalpy than Be, because -

  • It is easier to remove electrons from p - subshell than completely filled s - subshell.

  • The s-electron can be removed easier than the p electron.

  •  Ionisation enthalpy decreases with an increase in atomic number.

  •  Ionisation enthalpy increases along the period.

Difference between electron gain enthalphy and electronegativity is described by

  • Valence electrons

  • Atomic size

  • Atomic radii

  • Atomic number

Incorrect statement about metal is -
  • Metals can donate electrons.
  • Metals form ionic compounds.
  • Metals are more electronegative.
  • Metals have less ionization energy.

The group number that has metal, non-metal, liquid as well as gas at room temperature, is -

  • 15

  • 14

  • 18

  • 17

Elements ∆H1    ∆H2    ∆egH
    I    520   7300    -60
    II    419    3051   -48
   III    1681    3374   -328
   IV    1008   1846    -295
    V     2372     5251    +48
   VI      738     1451    -40
The least reactive element based on the above data is :
  • III
  • IV
  • II
  • V

Incorrect statement among the following is -

  • The p-block has 6 columns because a maximum of 6 electrons can occupy all the orbitals in a p-shell.

  • The d-block has 8 columns because a maximum of 8 electrons can occupy all the orbitals in a d-subshell.

  • Each block contains a number of columns equal to the number of electrons that can occupy that subshell.

  • The s- block contains mainly reactive metals.

Among the following elements, the one that is not an actinoid is:

  • Curium (Z=96)

  • Californium (Z=98)

  • Uranium (Z=92)

  • Terbium (Z=65)

The order of screening effect of electrons of s, p, d and f orbitals of a given shell of an atom on electrons in its outer shell is :

  • s > p > d > f

  • f > d > p > s

  • p < d < f < s

  • f > p > s > d

Among halogens, the correct order of amount of energy released in electron gain (electron gain enthalpy) is-

  • F > Cl > Br > I

  • F  < Cl < Br < I

  •  F<Cl>Br>I

  • F < Cl < Br < I

The period number in the long form of the periodic table is equal to : 

  • Magnetic quantum number of any element of the period.

  • Atomic number of any element of the period.

  • Maximum principal quantum number of any element of the period.

  • Maximum azimuthal quantum number of any element of the period.

The elements in which electrons are progressivelyfilled in 4f-orbitals are called:

  • Actinoids

  • Transition elements

  • Lanthanoids

  • Halogens

The correct order of size of the given species is: 

  •   I > I- > I+

  •   I+ > I- > I

  •   I > I+ > I-

  •   I- > I > I+

The outermost electronic configuration of the last element of the p-blockin the 6th period is represented by

  •  7s27p6

  •  5f146d107s27p0

  •  4f145d106s26p6

  •  4f145d106s26p4

Among the following elements whose atomic numbers are given below, which cannot be accommodated in

  • 107

  • 118

  • 126

  • 102

The elements with atomic numbers 35, 53, and 85 are

  • Noble gases

  • Halogens

  • Heavy metals

  • Light metals

The reactivity of alkali metals increases, whereas halogen decreases down the group, because -

  • On moving down, ionization enthalpy decreases in group 1 while the electron gain enthalpy becomes less negative in group 17.

  • On moving down, ionization enthalpy increases in group 1 while the electron gain enthalpy becomes less negative in group 17.

  • On moving down, ionization enthalpy increases in group 1 while the electron gain enthalpy becomes less positive in group 17.

  • On moving down, ionization enthalpy decreases in group 17 while the electron gain enthalpy becomes less negative in group 1.

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